Organic Chemistry-Package(Custom)
4th Edition
ISBN: 9781259141089
Author: SMITH
Publisher: MCG
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Chapter 1, Problem 1.22P
Interpretation Introduction
Interpretation: The conversion of given condensed structure of lactic acid to a Lewis structure is to be stated.
Concept introduction: To convert a condensed structure into Lewis structure, one should start from the left side and make sure that each carbon atom must be tetravalent. Also, give two lone pairs on each oxygen atom to have a complete octet.
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During periods of strenuous exercise, the buildup of lactic acid [CH3CH(OH)CO2H] causes the aching feeling in sore muscles. Convert this condensed structure to a Lewis structure of lactic acid.
During periods of strenuous exercise, the buildup of lactic acid [CH;CH(OH)CO,H] causes
the aching feeling in sore muscles. Convert this condensed structure to a Lewis structure
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Two or more of your answers are incorrect.
Use this condensed chemical structure to complete the table below.
O
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CH,=CH–C-H
The condensed chemical structure of acrolein
Some facts about the acrolein molecule:
number of carbon-carbon single (CC) bonds:
number of carbon-hydrogen single (CH) bonds:
number of lone pairs:
X
S
2
1
4
Chapter 1 Solutions
Organic Chemistry-Package(Custom)
Ch. 1 - While the most common isotope of nitrogen has a...Ch. 1 - Label each bond in the following compounds as...Ch. 1 - How many covalent bonds are predicted for each...Ch. 1 - Draw a valid Lewis structure for each species. a....Ch. 1 - Draw an acceptable Lewis structure for each...Ch. 1 - Prob. 1.6PCh. 1 - Draw a Lewis structure for each ion. a. CH3Ob....Ch. 1 - Draw Lewis structures for each molecular formula....Ch. 1 - Prob. 1.9PCh. 1 - Prob. 1.10P
Ch. 1 - Prob. 1.11PCh. 1 - Prob. 1.12PCh. 1 - Draw a second resonance structure for each...Ch. 1 - Prob. 1.14PCh. 1 - Draw a second resonance structure for nitrous...Ch. 1 - Prob. 1.16PCh. 1 - Prob. 1.17PCh. 1 - Prob. 1.18PCh. 1 - Prob. 1.19PCh. 1 - Prob. 1.20PCh. 1 - Simplify each condensed structure by using...Ch. 1 - Prob. 1.22PCh. 1 - Prob. 1.23PCh. 1 - Convert each skeletal structure to a complete...Ch. 1 - Draw in all hydrogens and lone pairs on the...Ch. 1 - Prob. 1.26PCh. 1 - What orbitals are used to form each of the CC, and...Ch. 1 - What orbitals are used to form each bond in the...Ch. 1 - Determine the hybridization around the highlighted...Ch. 1 - Classify each bond in the following molecules as ...Ch. 1 - Prob. 1.31PCh. 1 - Rank the following atoms in order of increasing...Ch. 1 - Prob. 1.33PCh. 1 - Prob. 1.34PCh. 1 - Provide the following information about...Ch. 1 - Use the ball-and-stick model to answer each...Ch. 1 - Citric acid is responsible for the tartness of...Ch. 1 - Zingerone gives ginger its pungent taste. a.What...Ch. 1 - Two radioactive isotopes of iodine used for the...Ch. 1 - Prob. 1.40PCh. 1 - Assign formal charges to each carbon atom in the...Ch. 1 - Assign formal charges to each N and O atom in the...Ch. 1 - Draw one valid Lewis structure for each compound....Ch. 1 - Prob. 1.44PCh. 1 - Prob. 1.45PCh. 1 - Prob. 1.46PCh. 1 - Draw all possible isomers for each molecular...Ch. 1 - 1.45 Draw Lewis structures for the nine isomers...Ch. 1 - Prob. 1.49PCh. 1 - Prob. 1.50PCh. 1 - Prob. 1.51PCh. 1 - Prob. 1.52PCh. 1 - Prob. 1.53PCh. 1 - Prob. 1.54PCh. 1 - Draw all reasonable resonance structures for each...Ch. 1 - Prob. 1.56PCh. 1 - Rank the resonance structures in each group in...Ch. 1 - 1.56 Consider the compounds and ions with curved...Ch. 1 - 1.57 Predict all bond angles in each...Ch. 1 - Predict the geometry around each indicated atom....Ch. 1 - Prob. 1.61PCh. 1 - Prob. 1.62PCh. 1 - Draw in all the carbon and hydrogen atoms in each...Ch. 1 - Prob. 1.64PCh. 1 - Prob. 1.65PCh. 1 - Prob. 1.66PCh. 1 - Prob. 1.67PCh. 1 - Each of the following condensed or skeletal...Ch. 1 - Prob. 1.69PCh. 1 - Prob. 1.70PCh. 1 - Prob. 1.71PCh. 1 - Prob. 1.72PCh. 1 - Prob. 1.73PCh. 1 - Prob. 1.74PCh. 1 - Two useful organic compounds that contain Cl atoms...Ch. 1 - Use the symbols + and to indicate the polarity of...Ch. 1 - Label the polar bonds in each molecule. Indicate...Ch. 1 - Answer the following questions about acetonitrile...Ch. 1 - Prob. 1.79PCh. 1 - The principles of this chapter can be applied to...Ch. 1 -
a. What is the hybridization of each N atom in...Ch. 1 - 1.77 Stalevo is the trade name for a medication...Ch. 1 - 1.78 and are two highly reactive carbon...Ch. 1 - 1.79 The N atom in (acetamide) is hybridized,...Ch. 1 - Prob. 1.85PCh. 1 - Prob. 1.86PCh. 1 - Prob. 1.87PCh. 1 - Prob. 1.88PCh. 1 - Prob. 1.89PCh. 1 - Prob. 1.90P
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- 2) Using bond energies, verify that the complete combustion of ethene gas, C2 H4 (g) (H2C = CH2), to gaseous carbon dioxide and the water is an exothermic reaction.arrow_forwardIs C3H7Br a polar molecule? If so, indicate the polarity of each bond and the direction of the net dipole.arrow_forwardStructural Isomers: In the next part you will learn a little about structural isomers and how to draw them. Structural isomers are compounds with the same molecular formula, but different bonding arrangements or connectivities. In other words, the atoms are connected in a different order. For example, there are 2 different compounds with the molecular formula C4H10. They are given below: H H-C- H -H H H HHH H- H H-C -H Η ΗΗ H H Do you see how the atoms are bonded in a different order in the 2 structures? So they are structural isomers. C3H12 Find three different molecular structures, isomers, with this formula. (Hint: Remember the C rule where every C atom needs to have 4 bonds.) C2H60 Find two different molecules with this formula. (Hint: What are the 2 ways you can C5H10 How many structural isomers can you find for this formula? (Hint: Notice that 2 H atoms have been removed. This means that there is EITHER 1 double bond OR there is a ring structure.) Try to provide at least 4…arrow_forward
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- Convert the condensed formula CH3(CH2), CHO into a Lewis structure (including all lone pair electrons). Click and drag to start drawing a structure. X 5 Aarrow_forwardWhich molecule contains carbon with a negative formal charge? CO CO2 H2CO CH4arrow_forwardWrite Lewis structures for these ions. Show all valence electrons and all formal charges. (a) Amide ion, NH2 (b) Bicarbonate ion, HCO3 (c) Carbonate ion, CO32 (d) Nitrate ion, NO3 (e) Formate ion, HCOO (f) Acetate ion, CH3COOarrow_forward
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